REQUIRED PRACTICAL 4 - ID tests Flashcards

(30 cards)

1
Q

Calcium Ca2+ flame colour

A

brick red

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2
Q

Strontium Sr2+ flame colour

A

Red

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3
Q

Barium Ba2+ flame colour

A

Pale green

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4
Q

Observation of halides with Acidified silver nitrate

A
  • Flouride = no ppt too soluble
  • Chloride = white ppt
  • Bromide = cream ppt
  • Iodide = yellow ppt
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5
Q

How to test for halides

A
  1. Dissolve spatula in measure of sample of dilute HNO3 and add few cm3 of dilute or conc ammonia
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6
Q

Observations of halides with DILUTE ammonia

A
  • Chloride = dissolves to form colourless solution
  • Bromide = ppt does not dissolve
  • Iodide = ppt does not dissolve
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7
Q

Observations of halides with CONC ammonia

A
  • Chloride dissolves to form colourless solution
  • Bromide = dissolves to form colourless solution
  • Iodide = ppt does not dissolve
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8
Q

Ionic equations for halides reactions with acidified silver nitrate

A
  • Ag+(aq) + Cl-(aq) —> AgCl(s)
  • Ag+(aq) + Br-(aq) —> AgBr(s)
  • Ag+(aq) + I-(aq) —> AgI(s)
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9
Q

Why does the silver nitrate solution have to be acidified?

A

To remove other ions which would interfere with the test like OH- or sulphite ions

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10
Q

Why is HCl acid not used to acidify the AgNO3 reaction

A

Cl- would react with silver ion Ag+ to form white ppt and form flase positive result

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11
Q

How to get pure dry sample of salt

A
  1. Filter to remove the solid from soluble products
  2. Wash to remove any insoluble purities
  3. Dry to remove water
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12
Q

Purity test

A
  • Melting point test
  • Pure substances melt at fixed melting point
  • Impure substances melt over range of temperatures
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13
Q

Trend down group 2 solubility with NaOH

A

Increases down group 2 (white ppt-> slight white ppt -> colourless solution)

Mg(OH)2 is insoluble

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14
Q

Barium chloride with any amount of NaOH

A

remains colourless

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15
Q

Magnesium chloride with NaOH

A
  • Colourless to slightly white ppt when limited NaOH used
  • Colourless to white ppt when excess used
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16
Q

Calcium bromide with any amount of NaOH

A

colourless –> slightly white ppt

17
Q

Strontium chloride with any amount of NaOH

A
  • Colourless to slightly white ppt
18
Q

Trend down group 2 solubility with H2SO4

A
  • solubility decreases
  • BaSO4 is white ppt and solubility increases down the group
19
Q

Barium chloride with any amount of H2SO4

20
Q

Strontium chloride with any amount of H2SO4

21
Q

Calcium bromide with any amount of H2SO4

A

Slight white ppt

22
Q

Magnesium chloride with H2SO4

A
  • With limited H2SO4 slightly white ppt
  • With excess remains colourless solution
23
Q

Test for ammonia solution

A
  • Place ammonium chloride + NaOH + warm releases NH3
  • Forms ammonia gas which is a weak base and turns damp red litmus paper blue
24
Q

Test for strong base (NaOH) and weak base (NH3 solution)

A
  • For both damp red litmus paper goes blue
  • Using a pH meter you will get a different reading NaOH = pH 13/14 and NH3 pH = 8-10
25
Test for carbonate ions CO3(2-) or HCO3-
* Add sample of hydrogen carbonate salt to acid and ensure the gas is bubbled into limewater * Effervescence and solid disappears * Turns cloudy if CO2 given off
26
Test for sulfates
* Dissolve sulfate salt in dilute HNO3 and add few cm3 of barium chloride * White ppt forms = BaSO4
27
KCL, KBr and KI with conc sulfuric acid
* KCl effervescence * KBr effervescence and brown gas produced, solution turns deep brown * KI solution goes deep brown immediately and brown gas produced
28
Paper test for KCl
Damp litmus paper turns red
29
Paper test for KBr
Damp K2Cr2O7 paper orange changes to green in presence of SO2 gas
30
Paper test for KI
Damp lead nitrate paper turns black in presence of H2S